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Instructions for an experiment on molecular models, focusing on drawing lewis structures for various compounds and determining their properties such as electronic geometry, molecular geometry, hybridization, polarity, and bond angle. The experiment includes examples of compounds like nh4+, bro4-, o3, n3-, brcl5, hno3, pocl3, and no2-, and requires the assignment of formal charges to resonance structures.
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Experiment 10- Dry lab - Molecular Models
(a) Total points for this Report/exercise = 10. All numbered problems are 1 pt each.
(b) You will submit this by yourself or you may work with other students in the lab. However, there can be
no more than three students and all students’ names must be written on this exercise.
(c) Submit the completed exercise by the end of this week by email.
(d) For all compounds draw the lewis structures clearly and underneath the structure indicate various
answers for questions 2-8.
(e) Make sure you address all questions given and show all work to be eligible for the maximum points
indicated for each question. Show and write all work only on the spaces provided after each
question. Since this is a Word doc, you can add space between questions if you need more space.
But under no circumstances are you to attach scratch sheets of paper!
Afterwards, you are to upload this file as a PDF.
a) Octet rule
b) Polar covalent bond
c) Resonance
d) Formal charge
e) VSEPR Theory
For questions 2-8, write the BEST Lewis dot structure for each molecule, being sure to give the electronic
geometry, molecular geometry, hybridization of the central element, polarity, and bond angle around the central
element.
structure is likely to contribute most to the correct structure of NO
or are they equivalent resonance structures.